Characteristics of the equilibrium constant

(1) The value of the equilibrium constant is independent of the original concentration of the reactants.

(2) The equilibrium constant has a definite value for every reaction at the particular temperature. Though, it varies with the change in temperature.

(3) For the reversible reaction, the equilibrium constant for forward reaction is inverse of equilibrium constant for the backward reaction

    In general, 

(4) The value of equilibrium constant tells the extent to which a reaction proceeds in the forward or reverse direction.

(5) The equilibrium constant is independent of the presence of catalyst.

(6) The value of equilibrium constant changes with the change in the temperature. Thermodynamically, it can be given that if  and  be the equilibrium constants of a reaction at absolute temperatures  and . If  ΔH is the heat of reaction at the constant volume, then we can state that

            (Van't Hoff equation)

Effect of the temperature can be studied in the below stated cases

(i) When  i.e. , neither heat is evolved nor absorbed

Therefore, equilibrium constant remains same at all temperatures.

(ii) When  ΔH = +ve that is when the heat is absorbed, reaction is endothermic. The temperature T₂ is higher than T₁.

The value of equilibrium constant is quite higher at higher temperature in case of the endothermic reactions.

(iii) When ΔH = - ve, i.e., heat is evolved, reaction is exothermic in nature. The temperature T₂ is higher than the temperature T₁.

The value of equilibrium constant is lower at the higher temperature in the case of the exothermic reactions.

(7) The value of equilibrium constant depends upon the stoichiometry of the chemical equation.

For the reaction

(i) Likewise, if a particular equation is multiplied by 2, equilibrium constant for the new reaction (K¢) will be the square of equilibrium constant (K) for original reaction that is K^' = K₂

(ii) If the chemical equation for a particular reaction is written in two steps having equilibrium constants K₁ and K₂, then equilibrium constants are related as K = K₁ * K₂

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